Practice 2
Practice 2a (Answers at the end)
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____ 1. When methanol undergoes complete combustion, the products are carbon dioxide and water.
__ CH3OH(λ) + __ O2(g) → __ CO2(g) + __ H2O(g)
What are the respective coefficients when the equation is balanced with the smallest whole numbers?
|a. |1, 1, 1, 1 |
|b. |1, 2, 1, 2 |
|c. |2, 2, 2, 4 |
|d. |2, 3, 2, 4 |
|e. |2, 4, 6, 4 |
____ 2. Metals react with oxygen to give oxides with the general formula MxOy. Write a balanced chemical equation for the reaction of iron with oxygen to yield iron(III) oxide.
|a. |Fe(s) + O2(g) → FeO2(s) |
|b. |2 Fe(s) + 3 O2(g) → Fe2O3(s) |
|c. |3 Fe(s) + O2(g) → Fe3O2(s) |
|d. |4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) |
|e. |6 Fe(s) + O2(g) → 2 Fe3O(s) |
____ 3. Calcium reacts with fluorine gas to produce calcium fluoride. How many moles of Ca will react with 1.0 moles of F2?
|a. |0.50 mol |
|b. |1.0 mol |
|c. |1.5 mol |
|d. |2.0 mol |
|e. |4.0 mol |
____ 4. Sodium carbonate reacts with hydrochloric acid as shown below in an unbalanced chemical equation. What mass of CO2 is produced from the reaction of 2.94 g Na2CO3 with excess HCl?
Na2CO3(s) + HCl(aq) → NaCl(aq) + CO2(g) + H2O(λ)
|a. |1.22 g |
|b. |2.44 g |
|c. |2.94 g |
|d. |5.88 g |
|e. |7.08 g |
____ 5. What is a correct method for determining how many grams of calcium oxide are produced in the reaction of 10.0 g calcium with excess oxygen?
2 Ca(s) + O2(g) → 2 CaO(s)
|a. |10.0 g Ca [pic][pic][pic]= |
|b. |10.0 g Ca [pic][pic][pic]= |
|c. |10.0 g Ca [pic][pic][pic]= |
|d. |10.0 g Ca [pic][pic][pic]= |
|e. |10.0 g Ca [pic][pic][pic]= |
____ 6. How many moles of potassium bromide can be produced from the reaction of 2.92 moles of potassium with 1.78 moles of bromine gas?
2 K(s) + Br2(g) → 2 KBr(s)
|a. |1.46 mol |
|b. |1.78 mol |
|c. |2.92 mol |
|d. |3.56 mol |
|e. |5.84 mol |
____ 7. Under certain conditions the formation of ammonia from nitrogen and hydrogen has a 7.82% yield. Under these conditions, how many grams of NH3 will be produced from the reaction 25.0 g N2 with 2.00 g H2?
N2(g) + 3 H2(g) → 2 NH3(g)
|a. |0.881 g |
|b. |2.37 g |
|c. |3.12 g |
|d. |11.3 g |
|e. |30.4 g |
____ 8. A mass of 2.052 g of a metal carbonate, MCO3, is heated to give the metal oxide and 0.4576 g CO2.
MCO3(s) → MO(s) + CO2(g)
What is the identity of the metal?
|a. |Cu |
|b. |Mg |
|c. |Ca |
|d. |Ba |
|e. |Co |
____ 9. A mixture of MgCO3 and MgCO3·3H2O has a mass of 3.057 g. After heating to drive off all the water the mass is 2.790 g. What is the mass percent of MgCO3·3H2O in the mixture?
|a. |22.4% |
|b. |43.2% |
|c. |67.0% |
|d. |77.6% |
|e. |91.3% |
____ 10. The combustion of 0.1703 mole of a hydrocarbon produces 12.27 g H2O and 22.48 g CO2. What is the molar mass of the hydrocarbon?
|a. |16.04 g/mol |
|b. |30.07 g/mol |
|c. |44.08 g/mol |
|d. |72.15 g/mol |
|e. |92.13 g/mol |
____ 11. Soft drink bottles are made of polyethylene terephthalate (PET), a polymer composed of carbon, hydrogen, and oxygen. If 4.375 g PET is burned in oxygen it produces 1.515 g H2O and 9.251 g CO2. What is the empirical formula for PET?
|a. |CHO |
|b. |CH7O5 |
|c. |C5H7O |
|d. |C8H10O |
|e. |C10H8O5 |
____ 12. Which of the following statements are correct?
|1. |All salts of carbonate ion are soluble in water. |
|2. |Most salts of chloride ion are soluble in water. |
|3. |All salts of hydroxide ion are soluble in water. |
|a. |1 only |
|b. |2 only |
|c. |3 only |
|d. |1 and 2 |
|e. |1, 2, and 3 |
____ 13. Which of the following compounds will be soluble in water: KNO3, Ca3(PO4)2, CuCl2, and Fe2S3?
|a. |KNO3 and Ca3(PO4)2 |
|b. |KNO3 and CuCl2 |
|c. |Ca3(PO4)2 and Fe2S3 |
|d. |CuCl2 and Fe2S3 |
|e. |KNO3, Ca3(PO4)2, and Fe2S3 |
____ 14. A white solid is either NaI or NaNO3. If an aqueous solution of the solid is prepared, the addition of which reagent will allow you to distinguish between the two compounds?
|a. |NaOH |
|b. |HCl |
|c. |K3PO4 |
|d. |NH4Br |
|e. |Pb(NO3)2 |
____ 15. What is the net ionic equation for the reaction of aqueous lead(II) nitrate with aqueous sodium bromide?
|a. |Pb(NO3)2(aq) + 2 NaBr(aq) → PbBr2(aq) + 2 NaNO3(s) |
|b. |Na+(aq) + NO3-(aq) → NaNO3(s) |
|c. |Pb2+(aq) + 2 Br-(aq) → PbBr2(s) |
|d. |Pb2+(aq) + 2 Na+(aq) → PbNa2(s) |
|e. |Pb(NO3)2(aq) + 2 NaBr(aq) → PbBr2(s) + 2 NaNO3(aq) |
____ 16. Which of the following compounds is a weak acid?
|a. |H3PO4 |
|b. |HI |
|c. |HBr |
|d. |HClO4 |
|e. |H2SO4 |
____ 17. Which of the following compounds is a weak base?
|a. |LiOH |
|b. |KCl |
|c. |CH3CO2H |
|d. |Sr(OH)2 |
|e. |NH3 |
____ 18. Which of the following species are strong acids: HNO3, HBr, H3PO4,CH3CO2H, and HSO4-?
|a. |HNO3 and HBr |
|b. |HNO3 and H3PO4 |
|c. |HBr and HSO4- |
|d. |H3PO4, CH3CO2H, and HSO4- |
|e. |HNO3, H3PO4, and HSO4- |
____ 19. Sulfuric acid is the product of the reaction of ____ and H2O.
|a. |H2S |
|b. |SO2 |
|c. |SO32- |
|d. |SO42- |
|e. |SO3 |
____ 20. Metal oxides react with water to produce ____.
|a. |hydrogen gas |
|b. |bases |
|c. |oxygen gas |
|d. |acids |
|e. |reduced metals |
____ 21. What is the net ionic equation for the reaction of aqueous lithium hydroxide and aqueous nitric acid?
|a. |H+(aq) + LiOH(aq) → H2O(λ) + Li+(aq) |
|b. |H+(aq) + OH-(aq) → H2O(λ) |
|c. |HNO3(aq) + LiOH(aq) → H2O(λ) + LiNO3(aq) |
|d. |Li+(aq) + NO3-(aq) → LiNO3(aq) |
|e. |LiOH(aq) + H2O(λ) → H+(aq) + Li(OH)2(s) |
____ 22. What are the spectator ions in the reaction between aqueous perchloric acid and aqueous potassium hydroxide?
|a. |H+, ClO4-, K+, and OH- |
|b. |H+ and OH- |
|c. |K+ and ClO4- |
|d. |H+ and ClO4- |
|e. |K+ and OH- |
____ 23. Write a net ionic equation for the reaction of aqueous acetic acid and aqueous potassium hydroxide.
|a. |CH3CO2H(aq) + KOH(aq) → K+(aq) + CH3CO2-(aq) + H2O(λ) |
|b. |CH3CO2H(aq) + KOH(aq) → KCH3CO2(aq) + H2O(λ) |
|c. |H+(aq) + OH-(aq) → H2O(λ) |
|d. |CH3CO2H(aq) + OH-(aq) → CH3CO3H2-(aq) |
|e. |CH3CO2H(aq) + OH-(aq) → CH3CO2-(aq) + H2O(λ) |
____ 24. One use of calcium oxide (lime) is in pollution control at coal-burning power plants. Which reaction below occurs in the smokestack of a power plant?
|a. |CaO(s) + C(s) → Ca(s) + CO(g) |
|b. |CaO(s) + SO3(g) → CaSO4(s) |
|c. |CaO(s) + SO3(g) → CaS(s) + 2 O2(g) |
|d. |2 CaO(s) + C(s) → Ca2C(s) + O2(g) |
|e. |CaO(s) + SO3(g) → Ca(s) + SO2(g) + O2(g) |
____ 25. Write a net ionic equation for the reaction of limestone and a strong acid.
|a. |Ca(s) + 2 H+(aq) → Ca2+(aq) + H2(g) |
|b. |CaCO3(s) + 2 H+(aq) → Ca2+(aq) + H2CO3(s) |
|c. |CaCO3(s) + 2 HCl(aq) → CaCl2(aq) + H2CO3(aq) |
|d. |CaCO3(s) + 2 H+(aq) → Ca2+(aq) + CO2(g) + H2O( λ) |
|e. |CaO(s) + 2 H+(aq) → Ca2+(aq) + H2O( λ) |
____ 26. Write a balanced equation for the reaction of aqueous solutions of baking soda and acetic acid.
|a. |NaHCO3(aq) + CH3CO2H(aq) → NaCH3CO2(aq) + H2O( λ) + CO2(g) |
|b. |2 NaHCO3(aq) + CH3CO2H(aq) → 2 Na2CO3(aq) + CH4(aq) + 2H2O( λ) + CO2(g) |
|c. |NaHCO3(aq) + CH3CO2H(aq) → H2CO3(s) + NaCH3CO2(aq) |
|d. |NaHCO3(aq) + CH3CO2H(aq) → NaOH(aq) + CH3CO2H(aq) + CO2(g) |
|e. |NaHCO3(aq) + CH3CO2H(aq) → CH4(aq) + 2 CO2(g) + O2(g) + NaOH(aq) |
____ 27. Write a balanced equation for the reaction of aqueous solutions of potassium sulfide and hydrochloric acid.
|a. |K2S(aq) + 2 HCl(aq) → 2 KH(aq) + SCl2(g) |
|b. |K2S(aq) + HCl(aq) → HS(g) + KCl(aq) |
|c. |K2S(aq) + 2 HCl(aq) → H2S(g) + 2 KCl(aq) |
|d. |K2S(aq) + 2 HCl(aq) → 2 K(s) + H2(g) + SCl2(g) |
|e. |K2S(aq) + 2 HCl(aq) → S(s) + H2(g) + 2 KCl(aq) |
____ 28. Which of the following chemical equations is an acid-base reaction?
|a. |2 HCl(aq) + Zn(s) → H2(g) + ZnCl2(aq) |
|b. |HCl(aq) + NH3(aq) → NH4Cl(aq) |
|c. |HCl(aq) + AgNO3(aq) → AgCl(s) + HNO3(aq) |
|d. |Ba(OH)2(aq) + Na2SO4(aq) → BaSO4(s) + 2 NaOH(aq) |
|e. |2 NaOH(aq) + CuCl2(aq) → Cu(OH)2(s) + 2 NaCl(aq) |
____ 29. Which molecule in the reaction below undergoes oxidation?
2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g)
|a. |C2H2 |
|b. |O2 |
|c. |H2O |
|d. |CO2 |
|e. |C2H2 and O2 |
____ 30. Which species in the reaction below undergoes reduction?
Sn(s) + 2 H+(aq) → Sn2+(aq) + H2(g)
|a. |Sn |
|b. |H+ |
|c. |Sn2+ |
|d. |H2 |
|e. |No compound is reduced. |
____ 31. Which compound is the oxidizing agent in the reaction below?
I-(aq) + ClO-(aq) → IO-(aq) + Cl-(aq)
|a. |I- |
|b. |H2O |
|c. |Cl- |
|d. |IO- |
|e. |ClO- |
____ 32. How many liters of 0.1107 M KCl(aq) contain 15.00 g of KCl?
|a. |0.02227 L |
|b. |0.5502 L |
|c. |1.661 L |
|d. |1.818 L |
|e. |123.8 L |
____ 33. If 0.3000 g of impure soda ash (Na2CO3) is titrated with 17.66 mL of 0.1187 M HCl, what is the percent purity of the soda ash?
Na2CO3(aq) + 2 HCl(aq) → 2 NaCl(aq) + H2O(λ) + CO2(g)
|a. |11.11% |
|b. |22.22% |
|c. |57.91% |
|d. |37.03% |
|e. |74.06% |
____ 34. Which one of the following statements is INCORRECT?
|a. |In an exothermic process heat is transferred from the system to the surroundings. |
|b. |The greater the heat capacity of an object, the more thermal energy it can store. |
|c. |The SI unit of specific heat capacity is joules per gram per Kelvin. |
|d. |The specific heat capacity has a positive value for liquids and a negative value for gases. |
|e. |When heat is transferred from the system to the surroundings, q is negative. |
____ 35. How much energy is required to change the temperature of 21.5 g Cu from 27.0 °C to 88.1 °C? The specific heat capacity of copper is 0.385 J/g·K.
|a. |223 J |
|b. |506 J |
|c. |641 J |
|d. |729 J |
|e. |3.41 × 103 J |
____ 36. When 27.0 g of an unknown metal at 88.4 °C is placed in 115 g H2O at 21.0 °C, the final temperature of the water is 23.7 °C. What is the specific heat capacity of the metal? The specific heat capacity of water is 4.184 J/g·K.
|a. |0.34 J/g·K |
|b. |0.51 J/g·K |
|c. |0.74 J/g·K |
|d. |0.94J/g·K |
|e. |1.4 J/g·K |
____ 37. Calculate the amount of heat required to change 50.0 g ice at -20.0 °C to steam at 135 °C. (Heat of fusion = 333 J/g; heat of vaporization = 2260 J/g; specific heat capacities: ice = 2.09 J/g·K, liquid water = 4.18 J/g·K, steam = 1.84 J/g·K)
|a. |4.18 kJ |
|b. |32.4 kJ |
|c. |78.8 kJ |
|d. |135 kJ |
|e. |156 kJ |
____ 38. Calculate ΔE for the system in which a gas absorbs 31 J of heat and does 18 J of work on the surroundings?
|a. |-49 J |
|b. |-13 J |
|c. |+13 J |
|d. |+31 J |
|e. |+49 J |
____ 39. The thermochemical equation for the combustion of butane is shown below.
C4H10(g) + 13/2 O2(g) → 4 CO2(g) + 5 H2O(λ) ΔH° = -2877 kJ
What is the enthalpy change for the following reaction?
16 CO2(g) + 20 H2O(λ) → 4 C4H10(g) + 26 O2(g)
|a. |-5754 kJ |
|b. |-719.2 kJ |
|c. |+719.2 kJ |
|d. |+5754 kJ |
|e. |+1.151 × 104 kJ |
____ 40. If 1.86 g MgO is combined with 100.0 mL of 1.00 M HCl (density 100.0 g/mL) in a coffee cup calorimeter, the temperature of the resulting solution increases from 21.3 °C to 35.7 °C. Calculate the enthalpy change for the reaction per mole of MgO. Assume that the specific heat capacity of the solution is 4.18 J/g·K.
|a. |-6.13 kJ |
|b. |-28.3 kJ |
|c. |-133 kJ |
|d. |-329 kJ |
|e. |-613 kJ |
____ 41. Calculate ΔH for the following reaction,
CaO(s) + CO2(g) → CaCO3(s)
given the thermochemical equations below.
2 Ca(s) + O2(g) → 2 CaO(s) ΔH = -1270.2 kJ
C(s) + O2(g) → CO2(g) ΔH = -393.5 kJ
2 Ca(s) + 2 C(s) + 3 O2(g) → 2 CaCO3(s) ΔH = -2413.8 kJ
|a. |-4077.3 kJ |
|b. |-750.1 kJ |
|c. |-178.3 kJ |
|d. |+350.2 kJ |
|e. |+2870.6 kJ |
____ 42. Which of the following chemical equations corresponds to the standard molar enthalpy of formation of N2O?
|a. |NO(g) + 1/2 N2(g) → N2O(g) |
|b. |N2(g) + 1/2 O2(g) → N2O(g) |
|c. |2N(g) + O(g) → N2O(g) |
|d. |N2(g) + O(g) → N2O(g) |
|e. |2 N2(g) + O2(g) → 2 N2O(g) |
____ 43. Calculate [pic] for the combustion of gaseous ethanol,
C2H5OH(g) + 3 O2(g) → 2 CO2(g) + 3 H2O(g)
using standard molar enthalpies of formation.
|molecule |[pic] (kJ/mol) |
|C2H5OH(g) |-235.3 |
|CO2(g) |-393.5 |
|H2O(g) |-241.8 |
|a. |-1747.7 kJ |
|b. |-1277.1 kJ |
|c. |-793.5 kJ |
|d. |-400.0 kJ |
|e. |-83.6 kJ |
____ 44. The standard enthalpy change for the combustion of 1 mole of benzene is -3267.4 kJ.
C6H6(λ) + 15/2 O2(g) → 6 CO2(g) + 3 H2O(λ)
Calculate [pic] for benzene based on the following standard molar enthalpies of formation.
|molecule |[pic] (kJ/mol) |
|CO2(g) |-393.5 |
|H2O(λ) |-285.8 |
|a. |-6485.8 kJ |
|b. |-3946.7 kJ |
|c. |-3218.4 kJ |
|d. |+49.0 kJ |
|e. |+2588.1 kJ |
____ 45. The standard molar enthalpy of formation of NH3(g) is -45.9 kJ/mol. What is the enthalpy change if 5.38 g N2(s) and 3.32 g H2(g) react to produce NH3(g)?
|a. |-75.6 kJ |
|b. |-50.4 kJ |
|c. |-17.6 kJ |
|d. |-8.81 kJ |
|e. |-1.20 kJ |
Practice 2a Answer Section
1. ANS: D OBJ: 4.2 Balancing Chemical Equations
2. ANS: D OBJ: 4.2 Balancing Chemical Equations
3. ANS: B OBJ: 4.3 Mass Relationships in Chemical Reactions: Stoichiometry
4. ANS: A OBJ: 4.3 Mass Relationships in Chemical Reactions: Stoichiometry
5. ANS: E OBJ: 4.3 Mass Relationships in Chemical Reactions: Stoichiometry
6. ANS: C OBJ: 4.4 Reactions in which One Reactant is Present in Limited Supply
7. ANS: B OBJ: 4.5 Percent Yield
8. ANS: D OBJ: 4.6 Chemical Equations and Chemical Analysis
9. ANS: A OBJ: 4.6 Chemical Equations and Chemical Analysis
10. ANS: C OBJ: 4.6 Chemical Equations and Chemical Analysis
11. ANS: E OBJ: 4.6 Chemical Equations and Chemical Analysis
12. ANS: B OBJ: 5.1 Properties of Compounds in Aqueous Solution
13. ANS: B OBJ: 5.1 Properties of Compounds in Aqueous Solution
14. ANS: E OBJ: 5.2 Precipitation Reactions
15. ANS: C OBJ: 5.2 Precipitation Reactions
16. ANS: A OBJ: 5.3 Acids and Bases
17. ANS: E OBJ: 5.3 Acids and Bases
18. ANS: A OBJ: 5.3 Acids and Bases
19. ANS: E OBJ: 5.3 Acids and Bases
20. ANS: B OBJ: 5.3 Acids and Bases
21. ANS: B OBJ: 5.4 Reactions of Acids and Bases
22. ANS: C OBJ: 5.4 Reactions of Acids and Bases
23. ANS: E OBJ: 5.4 Reactions of Acids and Bases
24. ANS: B OBJ: 5.4 Reactions of Acids and Bases
25. ANS: D OBJ: 5.5 Gas-Forming Reactions
26. ANS: A OBJ: 5.5 Gas-Forming Reactions
27. ANS: C OBJ: 5.5 Gas-Forming Reactions
28. ANS: B OBJ: 5.6 Classifying Reactions in Aqueous Solution
29. ANS: A OBJ: 5.7 Oxidation-Reduction Reactions
30. ANS: B OBJ: 5.7 Oxidation-Reduction Reactions
31. ANS: E OBJ: 5.7 Oxidation-Reduction Reactions
32. ANS: D OBJ: 5.8 Measuring Concentrations of Compounds in Solution
33. ANS: D OBJ: 5.10 Stoichiometry of Reactions in Aqueous Solution
34. ANS: D OBJ: 6.2 Specific Heat Capacity and Heat Transfer
35. ANS: B OBJ: 6.2 Specific Heat Capacity and Heat Transfer
36. ANS: C OBJ: 6.2 Specific Heat Capacity and Heat Transfer
37. ANS: E OBJ: 6.3 Energy and Changes of State
38. ANS: C OBJ: 6.4 The First Law of Thermodynamics
39. ANS: E OBJ: 6.5 Enthalpy Changes for Chemical Reactions
40. ANS: C OBJ: 6.5 Calorimetry
41. ANS: C OBJ: 6.7 Hess's Law
42. ANS: B OBJ: 6.8 Standard Enthalpies of Formation
43. ANS: B OBJ: 6.8 Standard Enthalpies of Formation
44. ANS: D OBJ: 6.8 Standard Enthalpies of Formation
45. ANS: C OBJ: 6.8 Standard Enthalpies of Formation
................
................
In order to avoid copyright disputes, this page is only a partial summary.
To fulfill the demand for quickly locating and searching documents.
It is intelligent file search solution for home and business.
Related searches
- physics chapter 2 practice test
- physics 2 practice tests
- sat 2 physics practice test
- ap physics 2 practice exam
- ochem 2 practice synthesis problems
- grade 2 practice book pdf
- psychology chapter 2 practice test
- psychology chapter 2 practice quiz
- math 2 subject test practice test
- 2 grade reading comprehension practice test
- 4 2 practice geometry answer key
- 7 2 practice worksheet answers